During an experiment, an ideal gas obeys an additional equation of state $P^2V = \text{constant}$. The initial temperature and volume of the gas are $T$ and $V$ respectively. When it expands to volume $2V$, its temperature will be:

An ideal gas expands according to the law $P^2 V = \text{constant}$. The internal energy of the gas

$A$ gas obeys the relation $P^2V = \text{constant}$. The initial temperature and volume are $T_0$ and $V_0$. If the gas expands to a volume $2V_0$, what will be its final temperature?

During an experiment, an ideal gas is found to obey a condition $VP^2 = \text{constant}$. The gas is initially at a temperature $T$, pressure $P$, and volume $V$. The gas expands to volume $4V$. Which of the following statements is correct?

In a process,temperature and volume of one mole of an ideal monoatomic gas are varied according to the relation $VT = K$,where $K$ is a constant. In this process,the temperature of the gas is increased by $\Delta T$. The amount of heat absorbed by the gas is ($R$ is the gas constant).

One mole of a monoatomic ideal gas is expanded by a process described by $p V^3 = C$,where $C$ is a constant. The heat capacity of the gas during the process is given by ($R$ is the gas constant).